Consider this reaction: →2NH3g+N2g3H2g At a certain temperature it obeys this rate law.rate =·16.0M−1s−1NH32 Suppose a vessel contains NH3 at a concentration of 1.15M. Calculate the concentration of NH3 in the vessel 0.720 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. =___M

Consider this reaction: 2SO3 (g) →2SO₂ (g) +0₂ (8) At a certain temperature it obeys this rate law. rate = (2.99 M¹.5-¹) [SO] Suppose a vessel contains SO3 at a concentration of 0.160 M. Calculate the concentration of SO3 in the vessel 24.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M 0 x10 X G

Consider this reaction: 2NH, (g) → N, (g) +3H, (g) At a certain temperature it obeys this rate law. 2 rate = (0.0581 Ms)[NH,1 Suppose a vessel contains NH, at a concentration of 1.39M. Calculate the concentration of NH, in the vessel 70.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 ?

Rate 3 = ______ molecules/(cm3·s)    Rate 4 =   ______ molecules/(cm3·s)

1. From the balanced equation, determine the rate of reaction with respect to [NOCI]. 2 NO(g) + Cl2(g) → 2 NOCI(g) 1 A[NOCI] A. Rate: = 2 At B. Rate = + C. Rate = D. Rate = 1 A[NOCI] 2 At 1 A[NO] 2 At 2 A[NOCI] At E. It is not possible to determine without more information.

8 H chemPad H XX LE # Supporting Materials Periodic Table Additional Materials W 17 - Su2... → Help Greek Constants and W The reaction of fluorine and chlorine dioxide, shown below, is first order with respect to fluorine and first order with respect to chlorine dioxide. Write the rate law for this reaction. (Rate expressions take the general form: rate = k. [A]a. [B]b.) F₂(g) + 2 CIO₂ (g) → 2 FCIO₂(g) Factors G b * webassign.net 8 Supplemental Data L a ▸ G

A student sets up two reactions Reaction 1 uses 0.250 mol/L of reactant, and Reaction 2 uses 0 500 mol/L of reactant. How many times faster is Reaction 2 compared to Reaction 12 Express your answer as a multiple of the rate for Reaction 1 to three significant figures. Note that Reaction 1 is already written for you, so just enter the number.

Consider this reaction: →H2CO3aq+H2OaqCO2aq At a certain temperature it obeys this rate law.rate =·0.0579M−1s−1H2CO32 Suppose a vessel contains H2CO3 at a concentration of 0.820M. Calculate the concentration of H2CO3 in the vessel 280.seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. =___M

A chemistry graduate student is studying the rate of this reaction: CICH, CH,CI (g) → CH,CHCI (g) + HC1 (g) She fills a reaction vessel with CICH,CH,Cl and measures its concentration as the reaction proceeds: [CICH,CH,CI] time (minutes) 0.600M 1.0 0.411 M 2.0 0.281 M 3.0 0.192M 4.0 0.132M Use this data to answer the following questions. Write the rate law for this reaction. rate = k Ox10 Calculate the value of the rate constant k. k = Round your answer to 2 significant digits. Also be の

2. Consider the reaction that occurs when a CIO2 solution and a solution containing hydroxide ions (OH) are mixed at 0°C, shown in the following equation. 2CIO2(aq) + 2OH (aq) → Cl03° (aq) + CIO2° (aq) + H2O (1) When solutions containing CIO2 and OH- in various concentrations were mixed at 0 oC, the following rate data were obtained: Determination Initial concentration Initial concentration of Initial rate for formation number of ClO2, mol/L OH", mol/L of CIO3¯ mol/Ls 1.25x10-2 1.30x10-3 2.33x10-4 2.50x10-2 1.30x10-3 9.34x104 3 2.50x10-2 2.60x103 1.87x10-3 a) Use the method of initial rates to find the order of the reaction with respect to CIO2 and with respect to OH. Write the rate equation for the reaction of CIO2 and OH´ at 0°C. b) Calculate the rate constant, k, for the reaction of clO2 and OH at 0°C. c) Calculate the reaction rate for the reaction CIO2 and OH at 0°C when the initial ClO2 and OH concentrations are 8.25x10-3 mol/L and 5.35x 10-² mol/L, respectively. 1.